Textbook-Integrated Guide to Educational Resources

TIGER

New Observations on the Copper-to-Silver-to-Gold DemonstrationDorin Bejan, Jeff Hastie, and Nigel J. BunceThis analysis of the classic copper-to-silver-to-gold demonstration describes the deposition of zinc in the form of the silver-colored alloy ?-brass, the evolution of hydrogen at the copper cathode, and the behavior of the associated electrochemical cell.Bejan, Dorin; Hastie, Jeff; Bunce, Nigel J. J. Chem. Educ.2008, 85, 1381.

Yet Another Variation on the Electrolysis of Water at Iron NailsMark T. Stauffer and Justin P. FoxDescribes a variation on the electrolysis of water with iron nails in which a sharp contrast in the colors produced effectively demonstrates electrolysis and the diffusion of oxidized and reduced species from the electrodes.Stauffer, Mark T.; Fox, Justin P. J. Chem. Educ.2008, 85, 523.

Electrochemical Polishing of Silverware: A Demonstration of Voltaic and Galvanic CellsMichelle M. Ivey and Eugene T. SmithUsing a battery and a graphite electrode, an electrolytic cell is constructed to generate a layer of tarnish on silverware. Students then determine that the tarnish can be removed by electrochemically converting it back to silver using aluminum foil and baking soda.Ivey, Michelle M.; Smith, Eugene T. J. Chem. Educ.2008, 85, 68.

Consumer Chemistry |

Electrochemistry |

Electrolytic / Galvanic Cells / Potentials

The Use of Conjugate Charts in Transfer Reactions: A Unified ApproachMichael I. AllnuttRedox reactions are discussed in terms of the relative strengths of the oxidant, the reductant, and their conjugates; a conjugate chart is a convenient and useful way of doing this. A similar chart for acids and bases that can be applied in the same manner is proposed.Allnutt, Michael I. J. Chem. Educ.2007, 84, 1659.

Photogalvanic Cells for Classroom Investigations: A Contribution for Ongoing Curriculum ModernizationClaudia Bohrmann-Linde and Michael W. TauschLaboratory experiments examining the fundamental processes in the conversion of light into electrical energy using photogalvanic cells have been developed. These simple cells are suitable for classroom investigations examining the operating principles of photogalvanic cells and the influence of different parameters on their efficiency. Bohrmann-Linde, Claudia; Tausch, Michael W. J. Chem. Educ.2003, 80, 1471.

Electrochemistry |

Atomic Properties / Structure |

Photochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials

Lithium Batteries: A Practical Application of Chemical PrinciplesRichard S. TreptowIn recent years batteries have emerged in the marketplace that take advantage of the unique properties of lithium. Lithium metal is an attractive choice to serve as a battery anode because it is easily oxidized and it produces an exceptionally high amount of electrical charge per unit-weight.Treptow, Richard S. J. Chem. Educ.2003, 80, 1015.

Consumer Chemistry |

Electrochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Lithium Batteries: A Practical Application of Chemical PrinciplesRichard S. TreptowIn recent years batteries have emerged in the marketplace that take advantage of the unique properties of lithium. Lithium metal is an attractive choice to serve as a battery anode because it is easily oxidized and it produces an exceptionally high amount of electrical charge per unit-weight.Treptow, Richard S. J. Chem. Educ.2003, 80, 1015.

Consumer Chemistry |

Electrochemistry |

Oxidation / Reduction |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Why Do Some Batteries Last Longer Than Others?Michael J. Smith and Colin A. VincentComparing the energy content of the cathode material of different commercial batteries using a test cell.Smith, Michael J.; Vincent, Colin A. J. Chem. Educ.2002, 79, 851.

Structure and Content of Some Primary BatteriesMichael J. Smith and Colin A. VincentAn experiment that complements electrochemical characterization and allows students to explore the structure of commercial cells and calculate the anode and cathode capacities from the stoichiometry of the cell reaction.Smith, Michael J.; Vincent, Colin A. J. Chem. Educ.2001, 78, 519.

Consumer Chemistry |

Electrochemistry |

Undergraduate Research |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Observations on Lemon CellsJerry GoodismanThe lemon cell, consisting of pieces of two different metals stuck into a lemon or other fruit, is pictured in many general chemistry textbooks without being discussed; manuscript describes simple experiments, suitable for the general chemistry laboratory, which elucidate how this kind of cell works. Goodisman, Jerry. J. Chem. Educ.2001, 78, 516.

Electrochemistry |

Metals |

Electrolytic / Galvanic Cells / Potentials

Understanding Electrochemical Thermodynamics through Entropy AnalysisThomas H. BindelThis discovery-based activity involves entropy analysis of galvanic cells. The intent of the activity is for students to discover the fundamentals of electrochemical cells through a combination of entropy analysis, exploration, and guided discovery. Bindel, Thomas H. J. Chem. Educ.2000, 77, 1031.

Electrochemistry |

Thermodynamics |

Electrolytic / Galvanic Cells / Potentials

Lemon Cells RevisitedRadhakrishnamurty, P.Analysis of the reactions and nature of the electrodes in the lemon cell.Radhakrishnamurty, P. J. Chem. Educ.1999, 76, 1190.

Electrochemistry |

Electrolytic / Galvanic Cells / Potentials |

Oxidation / Reduction

Slide Projector Corrosion CellSilvia Tejada, Estela Guevara, and Esperanza OlivaresThe process of corrosion can be demonstrated in a slide projector, since the cell is in the shape of a slide, or on the stage of an overhead projector by setting up a simple galvanic cell. Corrosion occurs as the result of a galvanic cell reaction, in which the corroding metal acts as the anode. Several simple demonstrations relating to corrosion are described here.Tejada, Silvia; Guevara, Estela; Olivares, Esperanza. J. Chem. Educ.1998, 75, 747.

Electrochemistry |

Microscale Lab |

Oxidation / Reduction |

Reactions |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Lemon Cells Revisited - The Lemon-Powered CalculatorDaniel J. Swartling and Charlotte MorganUsing lemons to create a voltaic cell to run items that students would use in their everyday lives drives home that chemistry plays an integral role in their lives. Swartling, Daniel J.; Morgan, Charlotte. J. Chem. Educ.1998, 75, 181.

The Comparative Performance of Batteries: The Lead-Acid and the Aluminum-Air CellsXavier LeRoux, Gerry A. Ottewill, and Frank C. WalshAn experimental program designed to convey, to students aged 16 through undergraduate, the principles of battery electrochemistry through a comparative study of two different systems, the lead acid cell and aluminum air cell, is described. LeRoux, Xavier; Ottewill, Gerry A.; Walsh, Frank C. J. Chem. Educ.1996, 73, 811.

Electrochemistry |

Electrolytic / Galvanic Cells / Potentials |

Applications of Chemistry

Demonstration of the Plasma StateJoachim P. Schreckenbach and Klaus RabendingImportant basic properties of the plasma state are recognized in a simple experimental arrangement described in this article.Schreckenbach, Joachim P.; Rabending, Klaus. J. Chem. Educ.1996, 73, 782.

Phases / Phase Transitions / Diagrams |

Conductivity |

Electrolytic / Galvanic Cells / Potentials

Work Done by a Chemical ReactionHenry BrouwerThe use of the "hot dog clock" has been the focus of discussions in a number of areas of electrochemistry. Included in these have been oxidation-reduction potentials, battery construction, salt bridges, electrolytes, and the concentration of ions in certain foods.Brouwer, Henry. J. Chem. Educ.1996, 73, 354.

Using the Biological Cell in Teaching ElectrochemistryMerkel, Eva Gankiewicz How electricity is produced in a simple cell is correlated with how commercial batteries work; this concept can then be related to how living cells send electrical impulses.Merkel, Eva Gankiewicz J. Chem. Educ.1994, 71, 240.

The anode and the sunrise.Mierzecki, Roman.Etymology of the terms anode and cathode.Mierzecki, Roman. J. Chem. Educ.1992, 69, 657.

Electrochemistry |

Electrolytic / Galvanic Cells / Potentials |

Nomenclature / Units / Symbols

The world's largest human salt bridgeSilverman, L. Phillip; Bunn, Barbara B.On a beautiful April afternoon, the 1500 students had fun and learned something about electrochemistry, and they helped set a world's record for the "Longest Human Salt Bridge".Silverman, L. Phillip; Bunn, Barbara B. J. Chem. Educ.1992, 69, 309.

Why the Daniell cell works!Martins, George F.The strength of bonds between atoms in metals, the relative ease of removing electrons from atoms, and the energy lowering of the attraction of water molecules for positive ions in solution all aid beginning student's understanding of why reactions occur.Martins, George F. J. Chem. Educ.1990, 67, 482.

Atomic Properties / Structure |

Metals |

Electrolytic / Galvanic Cells / Potentials

Redox reactions and the electropotential axis Vella, Alfred J.An introductory discussion should not get bogged down with the problems of representing cells by standard cell diagrams and notations and instead should concentrate on the chemistry of galvanic cells and the use of these cells in describing the concepts of redox chemistry.Vella, Alfred J. J. Chem. Educ.1990, 67, 479.

Using a projecting voltmeter to introduce voltaic cellsSolomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, AnthonyUsing a transparent "projecting" voltmeter and assembling a zinc versus copper cell one component at a time allows students to develop a more concrete notion of the nature of a voltaic cell and the potential it produces.Solomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, Anthony J. Chem. Educ.1989, 66, 510.

Experimental work with tin(II) chloride in a high school Sanchez, Manuela MartinThe author describes a final-project performed by students that integrates concepts of hydrolysis, Le Chatelier's principle, and electrolysis. Students seek answers to questions such as: "What reactions were involved; why is an aqueous solution of SnCl2 acidic; how can elemental tin be recovered from the system?" Sanchez, Manuela Martin J. Chem. Educ.1988, 65, 898.

A multi-topic problem for general chemistry Burness, James H.A 'marathon' problem which requires specific knowledge in several areas while requiring that the student recognize how these areas are related.Burness, James H. J. Chem. Educ.1988, 65, 145.

Car Won't Start?Nash, Leonard K.; Plumb, Robert C.Examines the questions, "Does the voltage of a battery drop with temperature" and "Does the ability of a battery to deliver current decrease with temperature?"Nash, Leonard K.; Plumb, Robert C. J. Chem. Educ.1970, 47, 382.

LettersHackney, J. C.The author elaborates on the source of a fallacy in the calculation of an overall redox potential by combination of two half-cell potentials.Hackney, J. C. J. Chem. Educ.1952, 29, 472.

Electrochemistry |

Electrolytic / Galvanic Cells / Potentials |

Aqueous Solution Chemistry |

Oxidation / Reduction

Miscellaneous experimentsDamerel, Charlotte I.Offers three demonstrations, the first involving molecular models illustrating the generation of optical isomers in a laboratory synthesis; the second demonstrating that liquid sodium chloride conducts and electric current; and the third examining the flow of electric current in an electrochemical galvanic cell.Damerel, Charlotte I. J. Chem. Educ.1952, 29, 296.